Chapter 5 Section 1 History of the Periodic Table pages 133-137 1 Modern Chemistry Chapter 5 The...

Chapter 5 Section 1 History of the Periodic Table pages 133-137

1

Modern ChemistryChapter 5

The Periodic Law

Sections 1-3History of the Periodic Table

Electron Configurations and the Periodic Table

Electron Configurations and Periodic Properties


2Chapter 5 Section 3 Periodic Properties pages 150-164

Electron Configurations and periodic properties

Section 3


3

Sect

ion 3

Voca

bula

ryAtomic radiusIonIonizationIonization EnergyElectron affinityCationAnionValence electronsElectronegativity

Chapter 5 Section 3 Periodic Properties pages 150-164


4

Atomic Radii• One half the distance between the nuclei

of identical atoms bonded together

Chapter 5 Section 3 Periodic Properties pages 150-164p.

150


5

Atomic Radii• Period Trend

– Atomic radii decreases across a period– Electrons are added to the s and p in

the same energy level– Protons are added to the nucleus– The nucleus is stronger and pulls in

the electrons making the atom smaller



6

Atomic Radii• Group Trend

– Atomic radii increases down a group– Exeption Al to Ga in group 13– Electrons exist in higher energy levels

further from the nucleus

Practice on page 152



7

Atomic radius imagep.

151

*



8

Ionization Energy • Ion: an atom or group of bonded

atoms that has a positive or negative charge

• Ionization: any process that results in the formation of an ion

• Ionization energy: The energy required to remove one electron from a neutral atom.



9

ion

anim

ati

on



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Ionization Energy • First ionization energy = IE1 (energy

to remove one electron)• Diagram on Page 153 and 154• A + energy A+ + e-



11

Ion

izait

on E

nerg

y C

om

icp.

## Chapter 5 Section 1 History of the

Periodic Table pages 133-137


12

Ion

izati

on e

nerg

y a

nim

ati

on



13

Ionization energy vs. atomic number graph

p. 1

54 Chapter 5 Section 1 History of the Periodic Table pages 133-137


14

Ionization Energy • Period Trend

– IE increases across a period– Increased nuclear charge holds e-

thighter– Elements with low IE lose e- easily– Elements with high IE do not lose e-– Generally nonmetals have higher IE

than metals



15

Ionization Energy • Group Trend

– IE decreases down a group– An electron is removed from higher

energy levels further from the nucleus– In elements with many electron, the

inner electrons in lower energy levels shield the outer electrons in the higher energy levels from the attraction of the nucleus



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Ionization energy imagep.

153

*


Dec

reas

e

Increase

Ionization Energy


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Ionization Energy • Removing electrons from positive ions

– More than one electron can be removed from an atom

– Second ionization energy = IE2 – IE2 is higher than IE1

– Because few electrons remain to shield the outer electrons from the nucleus

– Table on page 155

Practice page 156



18

1st- 5th Ionization energy chartp.

55 Chapter 5 Section 1 History of the

Periodic Table pages 133-137


19

Electron Affinity • The energy change that occurs when

an electron is acquired by a neutral atom

A + e- A- + energy orA + e- + energy A-

– Positive or less negative EA won’t likely gain electrons

– More negative EA will gain electrons easily Chapter 5 Section 3 Periodic

Properties pages 150-164

Energy is released negative number

Energy is absorbed positive number


20

Ele

ctro

n A

ffinit

y a

nim

ati

on



21

Electron affinity • Period Trend

– EA increases across the period (more neg.)

– Exception between group 14 and 16



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Electron affinity • Group Trend

– EA decreases down a group (less neg.)

– An increase in protons increases EA but an increase in radius decreases EA



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Electron Affinity imagep.

157

*


Dec

reas

e

Increase

Electron Affinity


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Electron affinity • Adding electrons to negative ions• More difficult to add a second

eletron• All second EA are positive



25

Ionic Radii • Positive Ions

– Cation– Loss of electron– Smaller electron cloud; loss of highest

energy level– Electrons are drawn closer to the

nucleusNa Na+



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Ionic Radii • Negative ion

– Anions– Gaining of electrons– The electron cloud spreads out

because of the repeling of electrons



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ions Cation - positive Anion - negative



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Ionic Radii • Period Trend

– Ionic radii decreases across a period– As protons increase the electrons

are pulled in



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Ionic Radii • Group Trend

– Ionic Radii increases down a group– More electrons in higher energy levels



30

Ionic RADIUS Imagep.

159

*



31

Valence electrons • Electrons available to be lost,

gained or shared in the formation of compounds.

• Located in the incompletely filled main energy level

• For main group elements – outer s & p sublevels



32

Vale

nce

ele

ctro

ns

an

imati

on

p. #

# Chapter 5 Section 1 History of the Periodic Table pages 133-137


33

electronegativity• A measure of an atom in a

compound to attract electrons from another atom in the compound

• Linus Pauling devised a scale from 0-4.

• Fluorine is the most electronegative EN = 4.0



34

Electronegativities

p.16

1 Chapter 5 Section 1 History of the Periodic Table pages 133-137


35

ele

ctro

negati

vit

y a

nim

ati

on



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electronegativity• Period Trend

– EN increases across a period– There are exceptions.



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electronegativity• Group Trend

– EN decreases down a group

Practice Page 162



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Electronegativityp.

160

*


Dec

reas

e

Increase

Electronegativity


39

Periodic Properties of the d and F block elements

• Many exceptions in atomic radii, IE, and EN

• Most d block elements from 2+ ions

• Group 3 from 3+ ions• Copper forms 1+ and 2+ ions• Iron forms 2+ and 3+ ions



40

Sum

mary

of

tren

ds

Imag

e



41

Section 3 Homework


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